Chemical Equilibrium online test as an assignmnet IIT JAM Notes | EduRev

IIT JAM : Chemical Equilibrium online test as an assignmnet IIT JAM Notes | EduRev

 Page 1


 
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009 
Mob. 011-47455430, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com 
Chemical Equilibrium Online Test (18
th
 Dec, 16) 
 
1. Consider the phase diagram given below:  
 
At the intersection point Q has phases that are in equilibrium are 
(a) Solid A, solid B and solid AB
2
.  (b) Solid A, solid AB
2
 and liquid 
(c) Solid B, solid AB
2
 and liquid  (d) Solid A, solid B, solid AB
2
 and 
liquid 
2. For the following equilibrium: calculate the equilibrium 
constant, if for the equilibrium, 
The equilibrium constant is 5.5 × 10
-10. 
(a) 1.8 × 10
-4
            (b) 1.8 × 10
-5
         (c) 1.8 ×10
-6
    (d) 1.8 ×10
-7 
 
3. The elevation in boiling point of a solution of 10 g of a binary electrolyte (molecular mass 
100) in 100 g of water is ? T
b
. The value of K
b
 for water is: 
(a)    (b) 10   (c) 1 0 ? T
b  
(d) 
 
 
4. For the reaction, if percentage dissociation of N
2
O
4
 are 25%, 50%, 
75% and 100%, then the sequence of observed vapour densities will be: 
(a) d
1
 > d
2
 > d
3
 > d
4     
(b) d
4
 > d
3
 > d
2
 > d
1
  
(c) d
1
 = d
2
 = d
3
 = d
4
           (d) (d
1
 = d
2
) > (d
3
 = d
4
)   
 
5. For the reaction, if the initial concentration of [H
2
] = [CO
2
] 
and x mol/litre of H
2
 is consumed at equilibrium, the correct expression of K
p
 is: 
(a)   (b)   (c)   (d) 
 
Page 2


 
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009 
Mob. 011-47455430, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com 
Chemical Equilibrium Online Test (18
th
 Dec, 16) 
 
1. Consider the phase diagram given below:  
 
At the intersection point Q has phases that are in equilibrium are 
(a) Solid A, solid B and solid AB
2
.  (b) Solid A, solid AB
2
 and liquid 
(c) Solid B, solid AB
2
 and liquid  (d) Solid A, solid B, solid AB
2
 and 
liquid 
2. For the following equilibrium: calculate the equilibrium 
constant, if for the equilibrium, 
The equilibrium constant is 5.5 × 10
-10. 
(a) 1.8 × 10
-4
            (b) 1.8 × 10
-5
         (c) 1.8 ×10
-6
    (d) 1.8 ×10
-7 
 
3. The elevation in boiling point of a solution of 10 g of a binary electrolyte (molecular mass 
100) in 100 g of water is ? T
b
. The value of K
b
 for water is: 
(a)    (b) 10   (c) 1 0 ? T
b  
(d) 
 
 
4. For the reaction, if percentage dissociation of N
2
O
4
 are 25%, 50%, 
75% and 100%, then the sequence of observed vapour densities will be: 
(a) d
1
 > d
2
 > d
3
 > d
4     
(b) d
4
 > d
3
 > d
2
 > d
1
  
(c) d
1
 = d
2
 = d
3
 = d
4
           (d) (d
1
 = d
2
) > (d
3
 = d
4
)   
 
5. For the reaction, if the initial concentration of [H
2
] = [CO
2
] 
and x mol/litre of H
2
 is consumed at equilibrium, the correct expression of K
p
 is: 
(a)   (b)   (c)   (d) 
 
 
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009 
Mob. 011-47455430, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com 
6. H
3
PO
4
 is a tribasic acid, it undergoes ionization as: 
 
Then, equilibrium constant for the followimg reaction will be: 
(a) K
1
K
2
K
3  
(b)
  
(c)
  
(d) 
7. The equilibrium constant for the reaction is 5. How many moles of CO
2
 must be added to 1 
litre container already containing 3 moles each of CO and H
2
O to make 2M equilibrium 
concentration of CO? 
(a) 15   (b) 19   (c) 5   (d) 20 
 
8. A nitrogen–hydrogen mixture initially in the molar ratio of 1:3 reacted equilibrium to form 
ammonia when 25% of the N
2
 and H
2
 had reached. If the total pressure of the system was 21 
atm, the partial pressure of ammonia at the equilibrium was: 
(a) 4.5 atm   (b) 3.0 atm  (c) 2.0 atm  (d) 1.5 atm 
 
9. The freezing point depression constant for water is 1.86°C m
–1
. If 5 g Na
2
SO
4
 is dissolved in 
45 g H
2
O, the freezing point is changed by –3.82°C. Calculate the van't Hoff factor for 
Na
2
SO
4.
  
(a) 0.381   (b) 2.05  (c) 2.63  (d) 3.11 
 
10. K
sp(AgCl)
 > K
sp(AgBr)
 > K
sp(AgI)
. This means that: 
(a) AgCl is more ionized than AgBr and AgI  
(b) Both AgBr & AgI are less soluble than AgCl 
(c) AgI is most soluble     
(d) AgBr is more soluble than AgCl but less soluble then AgI 
 
11. The triple point for water is: 
(a) Unique      (b) Depends on a p but is independent of T 
(c) Depends on T but is independent of P  (d) Depends on both P & T 
 
12. At 25°C, the volue of Pk
b
 (K
b
 being the dissociation constant as a base) for NH
3
 in aqueous 
solution is 4.7. What is the pH of 0.1 M aqueous solution of NH
4
Cl with 0.01 M 
NH
3
 (approxmately): 
Page 3


 
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009 
Mob. 011-47455430, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com 
Chemical Equilibrium Online Test (18
th
 Dec, 16) 
 
1. Consider the phase diagram given below:  
 
At the intersection point Q has phases that are in equilibrium are 
(a) Solid A, solid B and solid AB
2
.  (b) Solid A, solid AB
2
 and liquid 
(c) Solid B, solid AB
2
 and liquid  (d) Solid A, solid B, solid AB
2
 and 
liquid 
2. For the following equilibrium: calculate the equilibrium 
constant, if for the equilibrium, 
The equilibrium constant is 5.5 × 10
-10. 
(a) 1.8 × 10
-4
            (b) 1.8 × 10
-5
         (c) 1.8 ×10
-6
    (d) 1.8 ×10
-7 
 
3. The elevation in boiling point of a solution of 10 g of a binary electrolyte (molecular mass 
100) in 100 g of water is ? T
b
. The value of K
b
 for water is: 
(a)    (b) 10   (c) 1 0 ? T
b  
(d) 
 
 
4. For the reaction, if percentage dissociation of N
2
O
4
 are 25%, 50%, 
75% and 100%, then the sequence of observed vapour densities will be: 
(a) d
1
 > d
2
 > d
3
 > d
4     
(b) d
4
 > d
3
 > d
2
 > d
1
  
(c) d
1
 = d
2
 = d
3
 = d
4
           (d) (d
1
 = d
2
) > (d
3
 = d
4
)   
 
5. For the reaction, if the initial concentration of [H
2
] = [CO
2
] 
and x mol/litre of H
2
 is consumed at equilibrium, the correct expression of K
p
 is: 
(a)   (b)   (c)   (d) 
 
 
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009 
Mob. 011-47455430, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com 
6. H
3
PO
4
 is a tribasic acid, it undergoes ionization as: 
 
Then, equilibrium constant for the followimg reaction will be: 
(a) K
1
K
2
K
3  
(b)
  
(c)
  
(d) 
7. The equilibrium constant for the reaction is 5. How many moles of CO
2
 must be added to 1 
litre container already containing 3 moles each of CO and H
2
O to make 2M equilibrium 
concentration of CO? 
(a) 15   (b) 19   (c) 5   (d) 20 
 
8. A nitrogen–hydrogen mixture initially in the molar ratio of 1:3 reacted equilibrium to form 
ammonia when 25% of the N
2
 and H
2
 had reached. If the total pressure of the system was 21 
atm, the partial pressure of ammonia at the equilibrium was: 
(a) 4.5 atm   (b) 3.0 atm  (c) 2.0 atm  (d) 1.5 atm 
 
9. The freezing point depression constant for water is 1.86°C m
–1
. If 5 g Na
2
SO
4
 is dissolved in 
45 g H
2
O, the freezing point is changed by –3.82°C. Calculate the van't Hoff factor for 
Na
2
SO
4.
  
(a) 0.381   (b) 2.05  (c) 2.63  (d) 3.11 
 
10. K
sp(AgCl)
 > K
sp(AgBr)
 > K
sp(AgI)
. This means that: 
(a) AgCl is more ionized than AgBr and AgI  
(b) Both AgBr & AgI are less soluble than AgCl 
(c) AgI is most soluble     
(d) AgBr is more soluble than AgCl but less soluble then AgI 
 
11. The triple point for water is: 
(a) Unique      (b) Depends on a p but is independent of T 
(c) Depends on T but is independent of P  (d) Depends on both P & T 
 
12. At 25°C, the volue of Pk
b
 (K
b
 being the dissociation constant as a base) for NH
3
 in aqueous 
solution is 4.7. What is the pH of 0.1 M aqueous solution of NH
4
Cl with 0.01 M 
NH
3
 (approxmately): 
 
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009 
Mob. 011-47455430, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com 
(a) 8.3   (b) 9   (c) 9.5   (d) 10 
 
13. The solution of CaF
2
(K
sp
 = 3.4 × 10
–11
) in 0.1 M solution of NaF would be: 
(a) 3.4 × 10
–12
 M  (b) 3.4 × 10
–10
 M (c) 3.4 × 10
–9
 M (d) 3.4 × 10
–13
 M 
 
14. For the chemical equilibrium can be determined from which one of the following plots? 
(a)  (b) (c) (d) 
 
15. On adding 0.1 M solution each of Ag
+
, Ba
2+
 and Ca
2+ 
in an Na
2
SO
4
 solution, the species first 
precipitated is (K
sp
 BaSO
4
 = 10
–11
, K
sp
 CaSO
4
 = 10
–6
, K
sp
 Ag
2
SO
4
 = 10
–5
): 
(a) Ag
2
SO
4  
 (b) BaSO
4  
(c) CaSO
4  
(d) All of these 
 
16. Which of the following expression for % ionization of a mono-acidic base (BOH) in aqueous 
solution at appreciable concentration is correct? 
(a)     (b)  
(c)    (d)  
 
17. Which of the Following is/are affected by pressure change? 
(a) (b) 
(c)          (d) 
 
18. A buffer solution can be prepared from a mixture of? 
(a) Sodium acetate and acetic acid in water  
(b) Sodium acetate and HCl in water 
(c) Ammonia and ammonium chloride in water  
(d) Ammonia and sodium hydroxide in water. 
 
Page 4


 
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009 
Mob. 011-47455430, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com 
Chemical Equilibrium Online Test (18
th
 Dec, 16) 
 
1. Consider the phase diagram given below:  
 
At the intersection point Q has phases that are in equilibrium are 
(a) Solid A, solid B and solid AB
2
.  (b) Solid A, solid AB
2
 and liquid 
(c) Solid B, solid AB
2
 and liquid  (d) Solid A, solid B, solid AB
2
 and 
liquid 
2. For the following equilibrium: calculate the equilibrium 
constant, if for the equilibrium, 
The equilibrium constant is 5.5 × 10
-10. 
(a) 1.8 × 10
-4
            (b) 1.8 × 10
-5
         (c) 1.8 ×10
-6
    (d) 1.8 ×10
-7 
 
3. The elevation in boiling point of a solution of 10 g of a binary electrolyte (molecular mass 
100) in 100 g of water is ? T
b
. The value of K
b
 for water is: 
(a)    (b) 10   (c) 1 0 ? T
b  
(d) 
 
 
4. For the reaction, if percentage dissociation of N
2
O
4
 are 25%, 50%, 
75% and 100%, then the sequence of observed vapour densities will be: 
(a) d
1
 > d
2
 > d
3
 > d
4     
(b) d
4
 > d
3
 > d
2
 > d
1
  
(c) d
1
 = d
2
 = d
3
 = d
4
           (d) (d
1
 = d
2
) > (d
3
 = d
4
)   
 
5. For the reaction, if the initial concentration of [H
2
] = [CO
2
] 
and x mol/litre of H
2
 is consumed at equilibrium, the correct expression of K
p
 is: 
(a)   (b)   (c)   (d) 
 
 
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009 
Mob. 011-47455430, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com 
6. H
3
PO
4
 is a tribasic acid, it undergoes ionization as: 
 
Then, equilibrium constant for the followimg reaction will be: 
(a) K
1
K
2
K
3  
(b)
  
(c)
  
(d) 
7. The equilibrium constant for the reaction is 5. How many moles of CO
2
 must be added to 1 
litre container already containing 3 moles each of CO and H
2
O to make 2M equilibrium 
concentration of CO? 
(a) 15   (b) 19   (c) 5   (d) 20 
 
8. A nitrogen–hydrogen mixture initially in the molar ratio of 1:3 reacted equilibrium to form 
ammonia when 25% of the N
2
 and H
2
 had reached. If the total pressure of the system was 21 
atm, the partial pressure of ammonia at the equilibrium was: 
(a) 4.5 atm   (b) 3.0 atm  (c) 2.0 atm  (d) 1.5 atm 
 
9. The freezing point depression constant for water is 1.86°C m
–1
. If 5 g Na
2
SO
4
 is dissolved in 
45 g H
2
O, the freezing point is changed by –3.82°C. Calculate the van't Hoff factor for 
Na
2
SO
4.
  
(a) 0.381   (b) 2.05  (c) 2.63  (d) 3.11 
 
10. K
sp(AgCl)
 > K
sp(AgBr)
 > K
sp(AgI)
. This means that: 
(a) AgCl is more ionized than AgBr and AgI  
(b) Both AgBr & AgI are less soluble than AgCl 
(c) AgI is most soluble     
(d) AgBr is more soluble than AgCl but less soluble then AgI 
 
11. The triple point for water is: 
(a) Unique      (b) Depends on a p but is independent of T 
(c) Depends on T but is independent of P  (d) Depends on both P & T 
 
12. At 25°C, the volue of Pk
b
 (K
b
 being the dissociation constant as a base) for NH
3
 in aqueous 
solution is 4.7. What is the pH of 0.1 M aqueous solution of NH
4
Cl with 0.01 M 
NH
3
 (approxmately): 
 
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009 
Mob. 011-47455430, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com 
(a) 8.3   (b) 9   (c) 9.5   (d) 10 
 
13. The solution of CaF
2
(K
sp
 = 3.4 × 10
–11
) in 0.1 M solution of NaF would be: 
(a) 3.4 × 10
–12
 M  (b) 3.4 × 10
–10
 M (c) 3.4 × 10
–9
 M (d) 3.4 × 10
–13
 M 
 
14. For the chemical equilibrium can be determined from which one of the following plots? 
(a)  (b) (c) (d) 
 
15. On adding 0.1 M solution each of Ag
+
, Ba
2+
 and Ca
2+ 
in an Na
2
SO
4
 solution, the species first 
precipitated is (K
sp
 BaSO
4
 = 10
–11
, K
sp
 CaSO
4
 = 10
–6
, K
sp
 Ag
2
SO
4
 = 10
–5
): 
(a) Ag
2
SO
4  
 (b) BaSO
4  
(c) CaSO
4  
(d) All of these 
 
16. Which of the following expression for % ionization of a mono-acidic base (BOH) in aqueous 
solution at appreciable concentration is correct? 
(a)     (b)  
(c)    (d)  
 
17. Which of the Following is/are affected by pressure change? 
(a) (b) 
(c)          (d) 
 
18. A buffer solution can be prepared from a mixture of? 
(a) Sodium acetate and acetic acid in water  
(b) Sodium acetate and HCl in water 
(c) Ammonia and ammonium chloride in water  
(d) Ammonia and sodium hydroxide in water. 
 
 
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009 
Mob. 011-47455430, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com 
19. The equilibrium in aqueous medium at 25
0
C shifts towards the left in 
the presence of: 
(a) NO
3
-   
 (b) Cl
-
  (c) SCN
- 
  (d) CN
- 
 
20. Choose the correct statements: 
(a) pH of an acidic buffer increases if more salt is added 
(b) pH of a basic buffer decrease if more salt is added 
(c) In a saturated solution, ionic product is equal to its solubility product 
(d) The term solubility product is only for sparingly soluble salts 
 
21. The solubility of Pb(OH)
2
 in water is 6.7x10
-6
M. The solubility of Pb(OH)
2
 in a buffer solution 
of PH=8 is 1.2x10
-x
 what is the value of x. 
 
22.  3.1 mole of FeCl
3
 and 3.2 mole of NH
4
SCN are added tone litre of water. At equilibrium, 3.0 
mol of FeSCN
2+
 are formed. The equilibrium constant Kc of the reaction, 
 will be: 
 
23.  The equilibrium of formation of phosgene is represented as: 
 
The reaction is carried out in a 500 ml flask. At equilibrium 0.3 mole of phosgene, 0.1 mole of 
CO and 0.1 mole of Cl
2
 are present. The equilibrium constant of the reaction is: 
 
24. SO
3(g)
 is heated in a closed vessel. An equilibrium:  is established. 
The vapour density of the mixture, in which SO
3
 is 50% dissociated, is: 
 
25. The dissociation constant of a substituted benzoic acid at 25
0
C is 1.0x10
-4
. The PH of 0.01M 
solution of its sodium salt is. 
 
26. Consider the following reversible system: 
At equilibrium, there are 1.0 mole of A and 2.0 moles of each B,C 
& D present. If 2.0 mole of B is added further, how many moles of C would be required to be 
added so that mole of A & D do not change? 
 
 
 
Page 5


 
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009 
Mob. 011-47455430, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com 
Chemical Equilibrium Online Test (18
th
 Dec, 16) 
 
1. Consider the phase diagram given below:  
 
At the intersection point Q has phases that are in equilibrium are 
(a) Solid A, solid B and solid AB
2
.  (b) Solid A, solid AB
2
 and liquid 
(c) Solid B, solid AB
2
 and liquid  (d) Solid A, solid B, solid AB
2
 and 
liquid 
2. For the following equilibrium: calculate the equilibrium 
constant, if for the equilibrium, 
The equilibrium constant is 5.5 × 10
-10. 
(a) 1.8 × 10
-4
            (b) 1.8 × 10
-5
         (c) 1.8 ×10
-6
    (d) 1.8 ×10
-7 
 
3. The elevation in boiling point of a solution of 10 g of a binary electrolyte (molecular mass 
100) in 100 g of water is ? T
b
. The value of K
b
 for water is: 
(a)    (b) 10   (c) 1 0 ? T
b  
(d) 
 
 
4. For the reaction, if percentage dissociation of N
2
O
4
 are 25%, 50%, 
75% and 100%, then the sequence of observed vapour densities will be: 
(a) d
1
 > d
2
 > d
3
 > d
4     
(b) d
4
 > d
3
 > d
2
 > d
1
  
(c) d
1
 = d
2
 = d
3
 = d
4
           (d) (d
1
 = d
2
) > (d
3
 = d
4
)   
 
5. For the reaction, if the initial concentration of [H
2
] = [CO
2
] 
and x mol/litre of H
2
 is consumed at equilibrium, the correct expression of K
p
 is: 
(a)   (b)   (c)   (d) 
 
 
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009 
Mob. 011-47455430, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com 
6. H
3
PO
4
 is a tribasic acid, it undergoes ionization as: 
 
Then, equilibrium constant for the followimg reaction will be: 
(a) K
1
K
2
K
3  
(b)
  
(c)
  
(d) 
7. The equilibrium constant for the reaction is 5. How many moles of CO
2
 must be added to 1 
litre container already containing 3 moles each of CO and H
2
O to make 2M equilibrium 
concentration of CO? 
(a) 15   (b) 19   (c) 5   (d) 20 
 
8. A nitrogen–hydrogen mixture initially in the molar ratio of 1:3 reacted equilibrium to form 
ammonia when 25% of the N
2
 and H
2
 had reached. If the total pressure of the system was 21 
atm, the partial pressure of ammonia at the equilibrium was: 
(a) 4.5 atm   (b) 3.0 atm  (c) 2.0 atm  (d) 1.5 atm 
 
9. The freezing point depression constant for water is 1.86°C m
–1
. If 5 g Na
2
SO
4
 is dissolved in 
45 g H
2
O, the freezing point is changed by –3.82°C. Calculate the van't Hoff factor for 
Na
2
SO
4.
  
(a) 0.381   (b) 2.05  (c) 2.63  (d) 3.11 
 
10. K
sp(AgCl)
 > K
sp(AgBr)
 > K
sp(AgI)
. This means that: 
(a) AgCl is more ionized than AgBr and AgI  
(b) Both AgBr & AgI are less soluble than AgCl 
(c) AgI is most soluble     
(d) AgBr is more soluble than AgCl but less soluble then AgI 
 
11. The triple point for water is: 
(a) Unique      (b) Depends on a p but is independent of T 
(c) Depends on T but is independent of P  (d) Depends on both P & T 
 
12. At 25°C, the volue of Pk
b
 (K
b
 being the dissociation constant as a base) for NH
3
 in aqueous 
solution is 4.7. What is the pH of 0.1 M aqueous solution of NH
4
Cl with 0.01 M 
NH
3
 (approxmately): 
 
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009 
Mob. 011-47455430, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com 
(a) 8.3   (b) 9   (c) 9.5   (d) 10 
 
13. The solution of CaF
2
(K
sp
 = 3.4 × 10
–11
) in 0.1 M solution of NaF would be: 
(a) 3.4 × 10
–12
 M  (b) 3.4 × 10
–10
 M (c) 3.4 × 10
–9
 M (d) 3.4 × 10
–13
 M 
 
14. For the chemical equilibrium can be determined from which one of the following plots? 
(a)  (b) (c) (d) 
 
15. On adding 0.1 M solution each of Ag
+
, Ba
2+
 and Ca
2+ 
in an Na
2
SO
4
 solution, the species first 
precipitated is (K
sp
 BaSO
4
 = 10
–11
, K
sp
 CaSO
4
 = 10
–6
, K
sp
 Ag
2
SO
4
 = 10
–5
): 
(a) Ag
2
SO
4  
 (b) BaSO
4  
(c) CaSO
4  
(d) All of these 
 
16. Which of the following expression for % ionization of a mono-acidic base (BOH) in aqueous 
solution at appreciable concentration is correct? 
(a)     (b)  
(c)    (d)  
 
17. Which of the Following is/are affected by pressure change? 
(a) (b) 
(c)          (d) 
 
18. A buffer solution can be prepared from a mixture of? 
(a) Sodium acetate and acetic acid in water  
(b) Sodium acetate and HCl in water 
(c) Ammonia and ammonium chloride in water  
(d) Ammonia and sodium hydroxide in water. 
 
 
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009 
Mob. 011-47455430, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com 
19. The equilibrium in aqueous medium at 25
0
C shifts towards the left in 
the presence of: 
(a) NO
3
-   
 (b) Cl
-
  (c) SCN
- 
  (d) CN
- 
 
20. Choose the correct statements: 
(a) pH of an acidic buffer increases if more salt is added 
(b) pH of a basic buffer decrease if more salt is added 
(c) In a saturated solution, ionic product is equal to its solubility product 
(d) The term solubility product is only for sparingly soluble salts 
 
21. The solubility of Pb(OH)
2
 in water is 6.7x10
-6
M. The solubility of Pb(OH)
2
 in a buffer solution 
of PH=8 is 1.2x10
-x
 what is the value of x. 
 
22.  3.1 mole of FeCl
3
 and 3.2 mole of NH
4
SCN are added tone litre of water. At equilibrium, 3.0 
mol of FeSCN
2+
 are formed. The equilibrium constant Kc of the reaction, 
 will be: 
 
23.  The equilibrium of formation of phosgene is represented as: 
 
The reaction is carried out in a 500 ml flask. At equilibrium 0.3 mole of phosgene, 0.1 mole of 
CO and 0.1 mole of Cl
2
 are present. The equilibrium constant of the reaction is: 
 
24. SO
3(g)
 is heated in a closed vessel. An equilibrium:  is established. 
The vapour density of the mixture, in which SO
3
 is 50% dissociated, is: 
 
25. The dissociation constant of a substituted benzoic acid at 25
0
C is 1.0x10
-4
. The PH of 0.01M 
solution of its sodium salt is. 
 
26. Consider the following reversible system: 
At equilibrium, there are 1.0 mole of A and 2.0 moles of each B,C 
& D present. If 2.0 mole of B is added further, how many moles of C would be required to be 
added so that mole of A & D do not change? 
 
 
 
 
2637, Hudson Lane, Behind Khalsa College, Near G.T.B. Nagar Metro Station Gate No. 3 & 4, New Delhi – 110009 
Mob. 011-47455430, 08860929430, e-mail: info@asfinstitute.com, www.asfinstitute.com 
27. 0.10 mole each of SO
2
 and SO
3
 are mixed in a 2.0 dm
3 
flask at 300K. Equilibrium is attained 
as   
 
equilibrium pressure is 281.68 kpa. The mole fraction of O
2 
28. In the Reaction,  if D and d are the vapour densities at initial stage 
and at equilibrium then what will be the value of  at point A in the following graph? 
 
29. The number of degree of freedom of a system consisting of solid sucrose in equilibrium with 
an aqueous solution of sucrose is: 
 
30. 0.16 g of N
2
H
4
 are dissolved in water and the total volume made up to 500 mL. Calculate the 
percentage of N
2
H
4
 that has reacted with water at this dilution. The K
b
 for N
2
H
4
 is 4.0 × 10
–
6 
M: 
 
 
Answer key 
 
 
1.  c 2.  b  3.  a 4.  a 5.  a 
6.  a 7.  b 8.  b 9.  c 10.  b 
11.  d 12.  a 13.  c 14.  a 15.  a 
16.  a,b,d 17.  a,b,c,d 18.  a,b,c 19.  b,c,d 20.  a,b,c 
21.  3 22.  145 to 155 23.  15 24.   26 to 27 25.  8 
26.  6 27.  0.10 to 0.12 28.  1 29.  2 30.  2 
Read More
Offer running on EduRev: Apply code STAYHOME200 to get INR 200 off on our premium plan EduRev Infinity!

Complete Syllabus of IIT JAM

Content Category

Related Searches

Semester Notes

,

Chemical Equilibrium online test as an assignmnet IIT JAM Notes | EduRev

,

Previous Year Questions with Solutions

,

Exam

,

MCQs

,

pdf

,

practice quizzes

,

Sample Paper

,

ppt

,

Free

,

past year papers

,

shortcuts and tricks

,

Chemical Equilibrium online test as an assignmnet IIT JAM Notes | EduRev

,

Viva Questions

,

Extra Questions

,

Summary

,

study material

,

mock tests for examination

,

Important questions

,

video lectures

,

Chemical Equilibrium online test as an assignmnet IIT JAM Notes | EduRev

,

Objective type Questions

;